Given- Cs-O2g-CO2g- - H-395 kJ Ss-O2g-SO2g- H-295 kJ CS2l-3O2g-CO2g-2SO2g- H-1110 kJThe heat of formation of CS2l is-

The correct option is A 125 kJ Since, the formation reaction of CS_2 is, C(s) + 2S(s) → CS_2(l) Since, the formation reaction of CS_2 can ...

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Hess' Law

Given, Cs+O...

Question

Given,
$C (s) + O_{2} (g) \to {C O}_{2} (g); Δ H = - 395 k J$
$S (s) + O_{2} (g) \to {S O}_{2} (g); Δ H = - 295 k J$
$C S_{2} (l) + 3 O_{2} (g) \to {C O}_{2} (g) + 2 {S O}_{2} (g); Δ H = - 1110 k J$
The heat of formation of $C S_{2} (l)$ is:

250 k J

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62.5 k J

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31.25 k J

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125 k J

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Solution

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Given:

C(s) + O₂(g) → CO₂(g); ∆H = -395 kJ

S(s) + O₂(g) → SO₂(g); ∆H = -295 kJ

CS₂(l) + 3O₂(g) → CO₂(g) + 2 SO₂(g) ∆H = -1110 kJ

The heat of formation of CS₂(l) is

C_{(s)} + O_{2 (g)} \to C O_{2 (g)};

Δ H = - 394 k J

2 H_{2 (g)} + O_{2 (g)} \to 2 H_{2} O_{(l)};

Δ H = - 568 k J

C H_{4 (g)} + 2 O_{2 (g)} \to C O_{2 (g)} + 2 H_{2} O_{(l)};

Δ H = - 394 k J

C H_{4}

C (s) + O_{2} (g) \to C O_{2} (g); Δ H = - 94 k c a l

2 C O (g) + O_{2} (g) \to 2 C O_{2} (g); Δ H = - 135.2 k c a l

C O (g)

C (s) + O_{2} (g) \to {C O}_{2} (g); Δ H = r

C O (g) + \frac{1}{2} O_{2} (g) \to {C O}_{2} (g); Δ H = s

C O

C (s) + O_{2} (g) \to C O_{2} (g)

Δ H = - 394

2 H_{2} (g) + O_{2} (g) \to 2 H_{2} O (l), Δ H = - 568

C_{2} H_{5} O H (l) + 3 O_{2} (g) \to 2 C O_{2} (g) + 3 H_{2} O (l)

Δ H = - 1058

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